객관식
Which of the following elements has the largest ionization energy?
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10. Periodic Properties of the Elements
Periodic Trend: Ionization Energy
객관식
Which of the following atoms in the ground state requires the least amount of energy to remove its valence electron?
A
Na
B
Mg
C
Ca
D
K
검증된 단계별 안내1
Identify the elements given in the problem and their positions in the periodic table: Na (Sodium), Mg (Magnesium), Ca (Calcium), and K (Potassium).
Recall that the energy required to remove a valence electron is called the ionization energy, which generally decreases as you move down a group in the periodic table because the valence electron is farther from the nucleus and more shielded by inner electrons.
Compare the group and period of each element: Na and Mg are in period 3, Ca and K are in period 4, with K being in group 1 (alkali metals), Na also in group 1, Mg in group 2, and Ca in group 2.
Understand that elements in group 1 have lower ionization energies than those in group 2 because group 1 elements have only one valence electron, which is easier to remove.
Conclude that among the listed atoms, K (Potassium), being in group 1 and period 4, has the lowest ionization energy due to its larger atomic radius and weaker attraction to its valence electron, thus requiring the least energy to remove it.
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